Concept explainers
(a)
Interpretation:
Need to predict the shape of PCl5 according to the VSEPR theory.
Concept introduction:
Shapes of ions and molecules can be determined by VSEPR theory. This is valence shell electron pair repulsion theory and it is a model to predict the geometry of molecules from the amount of electron pairs around the central atom.
(b)
Interpretation:
Need to predict the shape of NH3 according to the VSEPR theory.
Concept introduction:
Shapes of ions and molecules can be determined by VSEPR theory. This is valence shell electron pair repulsion theory and it is a model to predict the geometry of molecules from the amount of electron pairs around the central atom.
(c)
Interpretation:
Need to predict the shape of ClF3 according to the VSEPR theory.
Concept introduction:
Shapes of ions and molecules can be determined by VSEPR theory. This is valence shell electron pair repulsion theory and it is a model to predict the geometry of molecules from the amount of electron pairs around the central atom.
(d)
Interpretation:
Need to predict the shape of SO2 according to the VSEPR theory.
Concept introduction:
Shapes of ions and molecules can be determined by VSEPR theory. This is valence shell electron pair repulsion theory and it is a model to predict the geometry of molecules from the amount of electron pairs around the central atom.
(e)
Interpretation:
Need to predict the shape of ClF4- according to the VSEPR theory.
Concept introduction:
Shapes of ions and molecules can be determined by VSEPR theory. This is valence shell electron pair repulsion theory and it is a model to predict the geometry of molecules from the amount of electron pairs around the central atom.
(f)
Interpretation:
Need to predict the shape of PCl4+ according to the VSEPR theory.
Concept introduction:
Shapes of ions and molecules can be determined by VSEPR theory. This is valence shell electron pair repulsion theory and it is a model to predict the geometry of molecules from the amount of electron pairs around the central atom.
Want to see the full answer?
Check out a sample textbook solutionChapter 10 Solutions
General Chemistry: Principles and Modern Applications (11th Edition)
- a. How many sticks did you need to make the skeleton structure?____________ b. How many sticks are left over? ____________ If your model is to obey the octet rule, each ball must have four sticks in it except for hydrogen atom balls, which need and can only have one. Each atom in an octet rule species is surrounded by four pairs of electrons. c. How many holes remain to be filled? ____________ Fill them with the remaining sticks, which represent nonbonding electron pairs. Draw the complete Lewis structure for NH2Cl using lines for bonds and pairs of dots for nonbonding electrons.arrow_forwardThink of forming an ionic compound as three steps (this is a simplification, as with all models): (I) removing an electron from the metal; (2) adding an electron to the nonmetal; and (3) allowing the metal cation and nonmetal anion to come together. a. What is the sign of the energy change for each of these three processes? b. In general, what is the sign of the sum of the first two processes? Use examples to support your answer. c. What must be the sign of the sum of the three process d. Given your answer to part c, why do ionic bonds occur? e. Given your above explanations, why is NaCl stable but not Na2Cl? NaCl2? What about MgO compared to MgO2? Mg2O?arrow_forwardIn Section 12.10 of your text, the term “effective pairs" is used. What does this mean?arrow_forward
- Distinguish between the terms electronegativity versus electron affinity, covalent bond versus ionic bond, and pure covalent bond versus polar covalent bond. Characterize the types of bonds in terms of electronegativity difference. Energetically, why do ionic and covalcnt bonds form?arrow_forwardWrite Lewis formulas for the BF molecule (two with a single BF bond, two with a double BF bond, and one with a triple BF bond) in which the octet rule is satisfied for at least one of the atoms. Obtain the formal charges of the atoms. Based on the information you have, is there one formula that you think best describes the molecule? Explain. For this best Lewis formula, give the valence bond description of the bonding.arrow_forwardConsider the molecular structures illustrated in the previous exercise. For each structure, give an example compound that has that arrangement of atoms.arrow_forward
- For three simple molecules of your own choice, apply the rules for writing Lewis structures. Write your discussion as if you are explaining the method to someone who is not familiar with Lewis structures.arrow_forwardBond Enthalpy When atoms of the hypothetical element X are placed together, they rapidly undergo reaction to form the X2 molecule: X(g)+X(g)X2(g) a Would you predict that this reaction is exothermic or endothermic? Explain. b Is the bond enthalpy of X2 a positive or a negative quantity? Why? c Suppose H for the reaction is 500 kJ/mol. Estimate the bond enthalpy of the X2 molecule. d Another hypothetical molecular compound, Y2(g), has a bond enthalpy of 750 kJ/mol, and the molecular compound XY(g) has a bond enthalpy of 1500 kJ/mol. Using bond enthalpy information, calculate H for the following reaction. X2(g)+Y2(g)2XY(g) e Given the following information, as well as the information previously presented, predict whether or not the hypothetical ionic compound AX is likely to form. In this compound, A forms the A+ cation, and X forms the X anion. Be sure to justify your answer. Reaction: A(g)+12X2(g)AX(s)The first ionization energy of A(g) is 400 kJ/mol. The electron affinity of X(g) is 525 kJ/mol. The lattice energy of AX(s) is 100 kJ/mol. f If you predicted that no ionic compound would form from the reaction in Part e, what minimum amount of AX(s) lattice energy might lead to compound formation?arrow_forward
- Chemical Principles in the LaboratoryChemistryISBN:9781305264434Author:Emil Slowinski, Wayne C. Wolsey, Robert RossiPublisher:Brooks Cole
- Chemistry: An Atoms First ApproachChemistryISBN:9781305079243Author:Steven S. Zumdahl, Susan A. ZumdahlPublisher:Cengage LearningChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage LearningGeneral Chemistry - Standalone book (MindTap Cour...ChemistryISBN:9781305580343Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; DarrellPublisher:Cengage Learning